Question

	pH	[H3O+]	[OH−]
0.1 L solution	2.5	3.2*10^-3	3.2*10^-12
1.0 L solution	3.50	3.2*10^-4	3.2*10^-11

Find the product of the [H₃O⁺] and the [OH⁻] for the 0.1 L solution.

Find the product of the [H₃O⁺] and the [OH⁻] for the 1.0 L solution.

Select the statement that best answers the following question

What is the relationship between [H₃O⁺] and [OH⁻] for the solutions?

1. The product of [H₃O⁺] and the [OH⁻] is greater for a solution with a higher pH.
2. The product of [H₃O⁺] and the [OH⁻] is lower for a solution with a higher pH.
3. The product of [H₃O⁺] and the [OH⁻] is constant for any pH.
4. The product of [H₃O⁺] and the [OH⁻] is not predictable, even if you know the pH.

between the solutions is a concentration and volume change by 10%. Why does the difference in pH make sense for this difference?

1. The pH is logarithmically related to concentration of H₃O⁺.
2. The pH is linearly related to concentration of H₃O⁺.
3. The pH is inversely proportional to the volume of the solution.
4. The pH increases as the volume of the solution increases.

Answer 1

Hope you will like my answer:)

0 1 Solution [Hot] = 3.2 X10S Product Els for the 0.1 L Solution 3 Con'] = 3,2 x10-12 M els CH2O] and 10-) is kwe Chot] [an] w? (3.2 x 10-12] [3.2 X 70-3] Kw = 1.024 X 10-14) 1*10 CHO * for the LOL solution [no] = 3.2 x 10-4 M row-1= 3.2 x 10-IM Product L CH0+ ] [on-] is *w = [H 0% ] [on-] Kw = (3.2x 10-4) x 13.2 X10-1) Kw=/1.024 x 10-14 r.ox 10-14 we have seen above that product of Inzot and con- is same for both olution independent of volume of solution and independent of concentration of individual Species [hot] & con-]. Product of (not] & [on-] is constant for any pH. Correct option is 0. T The given solutions have a conch and volume change by 10%. The change in pH is accounted as _= clost hot] on defends logarithmically on correct obrion ( not is @ . Scannedittramscanner